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Chemistry 121 > notes 23-34 > Flashcards

notes 23-34 Flashcards

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1
Q

Aufbau Principle

A

as protons are added on by one to the nucleus to build up the elements, electrons are similarly added to these hydrogen-like orbitals

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2
Q

Hund’s Rule

A

the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons (upe) allowed by the Pauli principle in a particular set of degenerate orbitals; generally shown as spin up

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3
Q

Pauli Exclusion Principle

A

no two electrons in an atom can have the same four numbers; electrons in the same orbital must have opposite spins

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4
Q

valence electrons (ve)

A

the electrons in the outermost principal quantum level of an atom

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5
Q

core electrons

A

inner electrons

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6
Q

Elements that have the same number of valence electrons…

A

…are in the same group which is why they have similar chemical reactivity.

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7
Q

Atomic Radius trend

A

atomic radii increases down a group and decreases across a period

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8
Q

Ionization Energy (IE)

A

the energy required to completely remove an electron from a gaseous atom or ion

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9
Q

Ionization Energy trend

A

IE decreases down a group and increases across a period (larger n → larger size → smaller IE)

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10
Q

Electron Affinity

A

the energy change associated with the addition of an electron to a gaseous atom

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11
Q

The greater the electron affinity…

A

…the greater the energy released when the electron is “captured” by the atom.

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12
Q

Electron Affinity trend

A

the electron affinity decreases (less negative) down a group and increases (more negative) across a period

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13
Q

Electron Affinity trend exceptions

A

He, Be, N, Ne, Mg, Ar

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14
Q

Size of Ions trend

A
  1. cations are smaller than the parent ion (removing electrons)
  2. anions are larger than the parent ion (adding electrons)
  3. ion size increases down a group
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15
Q

Isoelectronic Ions

A

ions containing the same number of electrons

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16
Q

Isoelectronic Ions trend

A

as atomic number increases the ionic radii decreases for an isoelectronic series

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17
Q

Paramagnetism

A

causes the substance to be attracted into an induced magnetic field; unpaired electrons

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18
Q

Diamagnetism

A

causes the substance to be repelled from an induced magnetic field; paired electrons

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19
Q

Metallic Character

A

metallic character increases down a group and decreases across a period

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20
Q

Bond Energy

A

the energy required to break a bond

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21
Q

ionic bonding

A

an atom loses electrons relatively easily and reacts with an atom that has a high affinity for that electron

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22
Q

covalent bonding

A

electrons are shared by two nuclei

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23
Q

polar covalent bonding

A

unequal sharing of electrons between two atoms

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24
Q

Electronegativity

A

the ability of an atom in a molecule to attract shared electrons to itself

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25
Q

Electronegativity trend

A

electronegativity decreases down a group and increases across a period; F has the highest electronegativity

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26
Q

dipole moment

A

a measure of the separation of positive and negative charge in a molecule

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27
Q

lattice energy

A

the change in energy that takes place when separated gaseous ions are packed together to form an ionic solid

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28
Q

single bond

A

a shared electron pair (sigma)

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29
Q

double bond

A

two shared electron pairs (sigma + pi)

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30
Q

triple bond

A

three shared electron pairs (sigma + 2pi)

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31
Q

C-C bond length

A

154pm

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32
Q

C=C bond length

A

134pm

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33
Q

C≡C bond length

A

120pm

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34
Q

enthalpy equation

A

ΔH = (sum of bonds broken) - (sum of bonds formed)

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35
Q

localized electron (LE) bonding model

A

a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms

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36
Q

lone pairs

A

pairs of electrons localized on an atom

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37
Q

bonding pairs

A

pairs of electrons found between atoms

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38
Q

Lewis structure

A

the arrangement of only the valence electrons in a molecule

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39
Q

duet rule

A

H forms stable molecules where it shares 2ve

40
Q

He doesn’t form bonds since…

A

…it already has 2ve (1s2)

41
Q

octet rule

A

the 2nd period forms bonds to fill all of its valence orbitals, tend to seek 8ve

42
Q

octet rule deficient

A

B, Be, Li

43
Q

elements that HAVE to follow the octet rule

A

C, N, O, F

44
Q

exceeds octet rule

A

elements in the 3rd period and larger

45
Q

resonance structures

A

multiple valid Lewis structures for a molecule; the average/combination of all of them is the correct structure

46
Q

formal charge

A

the difference between the # of valence electrons on the free atom and the # of ve assigned to the atom in the molecule

47
Q

molecular structure

A

the 3D arrangement of the atoms in a molecule

48
Q

sp hyrbidized

A

two effective pairs around an atom (one s and one p orbital)

49
Q

dsp3 hybridization

A

only happens when the octet is violated for the central atom (one d, one s, and three p orbitals)

50
Q

d2sp3 hybridization

A

six effective pairs around an atom; always arranged octahedrally

51
Q

weaknesses in the LE model

A

difficulty with uneven number of electrons, representing delocalized electrons, bond energy

52
Q

molecular orbital theory

A

an advanced model of chemical bonding in which electrons reside in molecular orbitals delocalized over the entire molecule. In the simplest version, the molecular orbitals are simply linear combinations of atomic orbitals

53
Q

MO1 is…
MO2 is…

A

…the sigma bond (bonding orbital)
…the sigma* bond (antibonding orbital)

54
Q

in the molecule the atomic orbitals no longer exist…

A

…only the MOs exist (new molecule → new orbitals)

55
Q

(bonding) MO1 is…
(antibonding) MO2 is…

A

… lower in energy than either of the two H 1s atomic orbitals
… higher in energy than either of the two H 1s atomic orbitals

56
Q

the MO labels show…

A

…shape, parent atomic orbitals, and bonding or antibonding

57
Q

bond order (BO)

A

the difference between the number of bonding electrons and the number of antibonding electrons divided by 2

58
Q

intramolecular forces

A

forces that bond atoms together to make molecules

59
Q

condensed states of matter

A

solids and liquids

60
Q

intermolecular forces

A

forces that hold the molecules together as aggregates

61
Q

gas

A

low density, indefinite shape, indefinite volume, weak IMF

62
Q

liquid

A

high density, indefinite shape, definite volume, moderate IMF

63
Q

solid

A

high density, definite shape, definite volume, strong IMF

64
Q

London Dispersion Forces (LDF)

A

the forces that exist between nonpolar molecules and atoms

65
Q

polarizability

A

a measure of how easily the electron cloud of an element can be distorted to give a dipolar charge distribution

66
Q

dipole-dipole attraction

A

molecules with dipole moments can line up +-+- to attract one another electrostatically

67
Q

hydrogen bonding

A

occurs in molecules that have hydrogen covalently bonded to highly electronegative atoms (H bonded to F, O, or N)

68
Q

ion-dipole forces

A

occur when ionic compounds are dissolved in polar substances

69
Q

surface tension

A

the resistance of a liquid to an increase in its surface area

70
Q

viscosity

A

a measure of a liquid’s resistance to flow

71
Q

capillary action

A

the spontaneous rising of a liquid in a narrow tube (cohesive + adhesive forces)

72
Q

cohesive forces

A

a result of the IMF among the molecules of the liquid

73
Q

adhesive forces

A

the forces between the liquid molecules and the container walls

74
Q

vaporization (evaporation)

A

when molecules or atoms of a liquid escape the liquid’s surface and form a gas

75
Q

enthalpy/heat of vaporization

A

the energy required to vaporize 1mol of a liquid at 1atm

76
Q

condensation

A

the process by which vapors reform a liquid

77
Q

vapor pressure

A

the pressure above the liquid in this closed system at this dynamic equilibrium

78
Q

volatile (VOC’s)

A

liquids with high vapor pressures

79
Q

non-volatile

A

liquids with low vapor pressures

80
Q

normal boiling point

A

the temperature at which the vapor pressure of the liquid is exactly 1atm

81
Q

boiling point

A

the temperature at which the vapor pressure of the liquid is equal to atmospheric pressure (changes with external pressure)

82
Q

Clausius-Clapeyron equation

A

y=mx+b

83
Q

sublimation

A

when a solid goes directly to the gaseous state without passing through the liquid state

84
Q

deposition (desublimation)

A

when a gas goes directly to the solid state without passing through the liquid state

85
Q

heating curve

A

a plot of temperature vs time for a process where energy is added as a constant rate

86
Q

enthalpy/heat of fusion

A

the enthalpy change that occurs at the melting point when a solid melts

87
Q

normal melting point

A

the temperature at which the solid and liquid states have the same vapor pressure under conditions where the total pressure is 1atm

88
Q

superheating

A

when a liquid is raised to a temperature above its boiling point without boiling

89
Q

sites of nucleation

A

molecular imperfection where molecules to accumulate

90
Q

bumping

A

once a bubble forms

91
Q

supercooling

A

cooled below its freezing point and remain a liquid

92
Q

cooling curve

A

a plot of temperature vs time for a process where energy is removed as a constant rate

93
Q

phase diagram

A

a convenient way of representing the phases of substance as a function of temperature and pressure

94
Q

critical temperature

A

the temperature above which the vapor cannot be liquefied no matter what pressure is applied (376ºC for water)

95
Q

critical pressure

A

the pressure required to produce liquefaction at the critical temperature (218atm for water)

96
Q

phase diagrams

A

a convenient way of representing the phases of a substance as a function of temperature and pressure

Chemistry 121 (6 decks)

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